Feb 8, 2017 · It is not yet clear how this “dissolved” oxygen should be described. Is it really dissolved in interstitial metal lattice positions, are there trapped $\ce{Au2O3}$ oxide clusters in a densely sintered metal matrix, or encapsulated oxygen gas …

Aug 20, 2022 · I keep reading that gold does not react with oxygen, but I also see information about gold Oxides (ie: aurous oxide, Au2O and auric oxide, Au2O3) Knowing that there is a way of getting gold oxide using multiple steps and additional chemicals (ie. decomposing aurous chloride), is there a way of getting gold oxide without any intermediate steps?

Mar 4, 2017 · $\ce{Au2O3}$ OS's That Don't Exist. The upper bound for OS's that you will meet is +7 for some manganese $(\ce{MnO4-})$, or chlorine $(\ce{ClO4-})$ compounds. OS's more than that are only found in exotic compounds. Thus, if you get a, say, +9 OS, you should start doubting the route you took. Determine the OS of W in $\ce{H4W2O13}$.

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Nov 20, 2018 · It seems that you have the answer, but I'll work it out anyways. Given the reaction: $$\ce{Cu(NH3)4^2+ + S2O4^2- -> SO3^2- + Cu + NH3}\tag{1}$$

Apr 5, 2018 · First of all, gold oxide cannot be obtained by reaction of gold and oxygen ($\ce{O2}$) at standard pressure. Gold oxide ($\ce{Au2O3}$) decomposes to gold and oxygen above $\pu{160°C}$. Ruthenium reacts with oxygen (air) above $\pu{700°C}$ to give $\ce{RuO4}$. Ruthenium powder burns in air.